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- A 1.000 g sample containing chlorides, iodides and inert materials was treated with dilute nitric acid followed by AgNO3. A precipitate of AgCl (143.32) and AgI (234.77) was produced and weighs 0.9238 g. On heating in a current of Cl2, the AgI is converted to AgCl, and the resulting product weighs 0.7238 g. Find the percentage of a) NaI (149.89) and b) NaCl (58.44) in the sample(c)Ions that react with Ag+ like SCN- can be determined electrogravimetricallyby deposition on a silver working anode:Ag(s) + SCN- ≤ AgSCN(s) + eA silver anode with initial mass of 12.4730 g was used to electrolyse 85.00 mL of asolution of 0.0245 M KSCN. At the end of the experiment, the anode weighed12.5767 g. How long did the experiment take, if a current of 100 mA was used?1. A Cr3+ solution is electrolyzed using a current of0.365 A. What mass of Cr(s) (51.9661) is plated outafter 10 hours?2. When an aqueous solution of CuSO4 is electrolyzedcopper metal is deposited. If a constant current waspassed for 5.00 h and 404 mg of Cu (63.546) metal wasdeposited, what was the current?
- (a) What is the percentage of MnO2 in a pyrolusite ore if a sample weighing 0.4000g is treated with 0.6000g of pure H2C2O4•2H2O and dilute H2SO4 and after reduction has taken place (MnO2 + H2C2O4 + 2H+→ Mn2++ 2CO2 + 2H2O), the excess oxalic acid requires 26.26ml of 0.1000N KMnO4 for titration? (b) If pure As2O3 were used instead of oxalic acid, how many grams would be required in order for the other numerical data to remain the same?The Sn in a 0.4352 g mineral specimen was reduced to the +2 state and titrated with 29.77 mL of 0.01735 M K2Cr2O7. Identify: (a) method of redox titrimetry used (Dichrometry, Cerimetry, iodimetry, iodometry or, permanganometry) (b) appropriate indicator and its type (c) color at the end point (d) weight percent Sn (118.71 g/mol) in the sampleCalculate the potential of a platinum electrode immersed in a solution that is (a) 0.0613 M in K4Fe(CN)6 and 0.00669 M inK3Fe(CN)6. E0=0.36 (b) 0.0400 M in FeSO4 and 0.00915 M in Fe2(SO4)3. E0=0.771 (c) buffered to a pH of 5.55 and saturated with H2 at 1.00 atm. (d) 0.1015 M in V(OH)4+, 0.0799 M in VO2+, and 0.0800 M in HClO4. E0=1 (e) prepared by mixing 50.00 mL of 0.0607 M Ce(SO4)2 with an equal volume of 0.100 M FeCl2 (assume solutions were 1.00 M in H2SO4 and use formal potentials).E0=0.68 (f ) prepared by mixing 25.00 mL of 0.0832 M V2(SO4)3 with 50.00 mL of 0.00628 M V(OH)4+ and has a pH of 1.00.
- 1.) A sodium sulfate solution was electrolyzed using inert Pt electrodes. The cathode reaction was 2H2O + H2+2OH^-. If a current of 3.0 amp was used for 30 min, what weight of H2O gas would be produced? 2.) What volume of H2 gas at STP would be produced during the passage of 30,000 Coul in the electrolysis of H2O? 3.) Give the notation for the cell that utilizes the reaction: (a) Cl2 (g)+ 2 I^-(aq) to 2 Cl^-(aq)+I2(s), (b) what is the E^o for the cell? (c) which electrode is the cathode? 4.) The standard electrode potential fornthe Fe^2+ to Fe^(3+) + e - half reaction is -0.770V. (a) Using the Nernst equation [E=E^o - (0.059/n) log [Oxid]/[Red]]. Calculate the voltage of this half cell when the [Fe^3+] is 1.0 x 10^-3 and [Fe^2+] is 1.0 x 10 ^ -1. (b) Calculate the approximate equilibrium constant (K) for the half reaction.When I was a boy, I watched Uncle Wilbur measure the iron content of runoff from his banana ranch. He acidified a 25.0-mL sample with HNO3 and treated it with excess KSCN to form a red complex. (KSCN itself is colorless.) He then diluted the solution to 100.0 mL and put it in a variablepathlength cell. For comparison, he treated a 10.0-mL reference sample of 6.80X 1024 M Fe31 with HNO3 and KSCN and diluted it to 50.0 mL. The reference was placed in a cell with a 1.00-cm pathlength. Runoff had the same absorbance as the reference when the pathlength of the runoff cell was 2.48 cm. What was the concentration of iron in Uncle Wilbur’s runoff ?A dilute solution of CuSO4 was electrolyzed using Pt- electrodes. The amount of Cu in the anodic solution was found to be 0.6350 g and 0.6236 g before and after electrolysis, respectively. The weight of Ag deposited in a silver coulometer, placed in series, was found to be 0.1351 g. Calculate the transport numbers of Cu+2 and SO4-2.
- Many applications of electrochemistry have been in chemical analysis.Suppose a Fe|Fe2+ concentration cell is set-up in which the [Fe2+] = 1.0 x10¯2 M in one compartment but the concentration in the othercompartment is unknown. The Ecell was measured at 0.024V when thehalf-cells were connected.(i) Without doing a numerical calculation, is the unknown more orless concentrated than the 1.0 x 10¯2 M solution? Justify youranswerIn a polarographic experiment of a 60 mL of 0.08 M Cu2+solution, a limitingcurrent was left on for 15 minutes. If the average current during the time of theexperiment is 6.0 μA, what fraction of the copper is removed from the solution? TheFaraday constant is 96485 C/mol of electron.Pyrolusite (MnO2) is dissolved in hydrochloric acid:MnO2 + HCl → MnCl2 + H2O + Cl2The chloride was passed into potassium iodide solution where it liberated iodine:Cl2 + KI → KCl + I2The iodine liberated was estimated by adding sodium thiosulfate, the reaction beingI2 + Na2S2O3 → NaI + Na2S4O6If 5.6 g of crystallized sodium thiosulfate, Na2S2O3 5H2O ,were used up, how many grams of manganese were present?MW (g/mole): I =126.9; Mn =54.94; Cl = 35.45; K = 39.09; Na = 23; S = 32